Answer:
They would all exhibit the same pressure.
Explanation:
Since the same number of mole of each gas is placed in different containers, it means the gas will occupy the same volume.
Now, the gases were observed at the same temperature. This means they will all have the same pressure as their volume is the same.
Now we can further understand this by doing a simple calculation as follow:
Assumptions:
For H2:
Number of mole (n) = 1 mole
Volume (V) = 22.4L
Temperature (T) = 298K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure =..?
PV = nRT
Divide both side V
P = nRT /V
P = 1 x 0.0821 x 298 / 22.4
P = 1 atm
Therefore, H2 has a pressure of 1 atm.
For N2:
Number of mole (n) = 1 mole
Volume (V) = 22.4L
Temperature (T) = 298K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure =..?
PV = nRT
Divide both side V
P = nRT /V
P = 1 x 0.0821 x 298 / 22.4
P = 1 atm
Therefore, N2 has a pressure of 1 atm
For O2:
Number of mole (n) = 1 mole
Volume (V) = 22.4L
Temperature (T) = 298K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure =..?
PV = nRT
Divide both side V
P = nRT /V
P = 1 x 0.0821 x 298 / 22.4
P = 1 atm
Therefore, O2 has a pressure of 1 atm
For He:
Number of mole (n) = 1 mole
Volume (V) = 22.4L
Temperature (T) = 298K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure =..?
PV = nRT
Divide both side V
P = nRT /V
P = 1 x 0.0821 x 298 / 22.4
P = 1 atm
Therefore, He has a pressure of 1 atm.
From the above illustrations we can see that the gases have the same pressure since they have the same number of mole, volume and were observed at the same temperature.
